4) A 2.234 x 10-6 M solution of HI (hydroiodic acid).
5) A 7.98 x 10-2 M solution of HNO3 (nitric acid).
6) 12 L of a solution containing 1 mole of hydrochloric acid.
7) 735 L of a solution containing 0.34 moles of nitric acid.
8) 1098 L of a solution containing 8.543 moles of hydrobromic acid.
9) 660 L of a solution containing .0074 moles of hydrochloric acid.
10) 120 mL of a solution containing 0.005 grams of hydrochloric acid.
11) 1.2 L of a solution containing 5.0 x 10-4 grams of hydrobromic acid.
12) 2.3 L of a solution containing 4.5 grams of nitric acid.
13) 792 mL of a solution containing 0.344 grams of hydrochloric acid.
14) 100 mL of a solution containing 1.00 grams of nitric acid.
15) 8.7 L of a solution containing 1.1 grams of nitric acid.
16) 1.5 L of a solution containing 5.6 grams of hydroiodic acid.
17) 10.7 L of a solution containing 0.01 grams of hydrochloric acid.
18) 8,000 L of a solution containing 6.7 grams of nitric acid and 4.5 grams of hydrochloric acid.
19) 150,000 L of a solution containing 45 grams of nitric acid and 998 grams of hydrobromic acid.
20) 50 L of a solution containing 0.09 grams of HCl, 0.9 grams of HBr, 9.0 grams of HI, and 90.0 grams of HNO3.
Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the following acid-base reactions and indicate each conjugate acid-base pair:
Time Length
- 2 Days
InstructionspH Calculations
Find the pH of the following acidic solutions:
1) A 0.001 M solution of HCl (hydrochloric acid).
2) A 0.09 M solution of HBr (hydrobromic acid).
3) A 1.34 x 10-4 M solution of hydrochloric acid.
4) A 2.234 x 10-6 M solution of HI (hydroiodic acid).
5) A 7.98 x 10-2 M solution of HNO3 (nitric acid).
6) 12 L of a solution containing 1 mole of hydrochloric acid.
7) 735 L of a solution containing 0.34 moles of nitric acid.
8) 1098 L of a solution containing 8.543 moles of hydrobromic acid.
9) 660 L of a solution containing .0074 moles of hydrochloric acid.
10) 120 mL of a solution containing 0.005 grams of hydrochloric acid.
11) 1.2 L of a solution containing 5.0 x 10-4 grams of hydrobromic acid.
12) 2.3 L of a solution containing 4.5 grams of nitric acid.
13) 792 mL of a solution containing 0.344 grams of hydrochloric acid.
14) 100 mL of a solution containing 1.00 grams of nitric acid.
15) 8.7 L of a solution containing 1.1 grams of nitric acid.
16) 1.5 L of a solution containing 5.6 grams of hydroiodic acid.
17) 10.7 L of a solution containing 0.01 grams of hydrochloric acid.
18) 8,000 L of a solution containing 6.7 grams of nitric acid and 4.5 grams of hydrochloric acid.
19) 150,000 L of a solution containing 45 grams of nitric acid and 998 grams of hydrobromic acid.
20) 50 L of a solution containing 0.09 grams of HCl, 0.9 grams of HBr, 9.0 grams of HI, and 90.0 grams of HNO3.
Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the following acid-base reactions and indicate each conjugate acid-base pair:
a) HNO3 + OH- à
b) CH3NH2 + H2O à
c) OH- + HPO4-2 à